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Review Periodic table, Isotopes, Ions.

Total questions: 70

Worksheet time: 23mins

Name
Class
Date
1.

Elements are arranged in decreasing order of atomic numbers in the Periodic Table.

a)

T

b)

F

2.

The group number of an atom is equal to the number of outermost shell electrons in the atom.

a)

T

b)

F

3.

Group VII elements are known as noble gases.

a)

T

b)

F

4.
a)
Periods
b)
Groups
5.
a)
Periods
b)
Groups
6.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
7.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
8.
a)
Same group
b)
Same period
9.
a)
Group 1
b)
Group 17
c)
Group 2
d)
Group 18
10.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
11.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
12.
a)
Metals
b)
Nonmetals
c)
Metalloids
13.
a)
Metals
b)
Nonmetals
c)
Metalloids
14.
a)
Metals
b)
Nonmetals
c)
Metalloids
15.
a)
Metals
b)
Nonmetals
c)
Metalloids
16.
a)
Metals
b)
Nonmetals
c)
Metalloids
17.
a)
Metals
b)
Nonmetals
c)
Metalloids
18.
a)
Metals
b)
Nonmetals
c)
Metalloids
19.
a)
Metals
b)
Nonmetals
c)
Metalloids
20.
What group does this element belong to?
a)
Group 1: Alkali metals
b)
Group 18: Noble Gases
c)
Group 2: Alkaline-Earth Metals
d)
Group 17: Halogens
21.

Select all the ions

a)

Na+

b)

Ba

c)

Po

d)

At-

e)

Fr+

22.

Magnesium has an atomic number of 12 and is in group 2. As a magnesium ion, what is its charge?

a)

2+

b)

+

c)

-

d)

2-

23.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
24.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
25.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
26.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
27.
Which of these elements has an electron structure most similar to that of element X?
a)
1
b)
2
c)
3
d)
4
28.
All elements found on the left side of the Periodic Table of the Elements have what properties in common?
a)
They conduct heat and electricity 
b)
They are all gases 
c)
They are brittle and dull
d)
They are radioactive
29.
Which element has 2 valence electrons? 
a)
cesium (Cs) 
b)
magnesium (Mg)
c)
boron (B)
d)
argon (Ar) 
30.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
31.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
32.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
33.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
34.

According to Coulomb's Law, when the distance increases, the electrostatic force ____________; we call this relationship ____________ proportional.

a)

decreases; directly

b)

decreases; inversely

c)

increases; inversely

d)

increases; directly

35.

Coulomb’s law states that the force between two charged objects will __________ when the magnitude (value) of the object’s charge increases.

a)

increase

b)

decrease

c)

stay the same

d)

first increase, then decrease

36.

Select all answer that apply:


What kinds of particles do Coulomb's Law apply to?

a)

electrons

b)

protons

c)

neutrons

d)

neutral atoms

37.

A repulsive force exists between which two particles?

a)

Two neutrons

b)

An electron and a neutron

c)

An electron and a proton

d)

Two protons

38.

An attractive force exists between which two particles?

a)

Two neutrons

b)

An electron and a neutron

c)

An electron and a proton

d)

Two electrons

39.

What does "r" measure?

a)

the distance between the two charged objects

b)

the amount of charge carried by the objects

c)

the amount of force between two charged objects

d)

the constant value for forces between the objects

40.
When distance increases, electrostatic force ____________; we call this relationship ____________ proportional
a)
decreases;directly
b)
decreases;inversely
c)
increases;inversely
d)
increases;directly
41.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

42.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

43.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

44.

How do you calculate mass number?

a)

Mass x percent

b)

Protons + Electrons

c)

Protons + Neutrons

d)

Neutrons + Protons + Electrons

45.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

46.

What is the ion formed from Sulfur? If it has 6 valence electrons.

a)

S+2

b)

S-2

c)

S+6

d)

S-6

47.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

48.
How many shielding electrons does carbon have? (hint: write its configuration first)
a)
1
b)
2
c)
3
d)
4
49.
How many valence electrons does carbon have?
a)
3
b)
4
c)
5
d)
6
50.
As you go down a group, the amount of shielding....
a)
increases
b)
decreases
c)
stays the same
51.
As you go across a period, the amount of shielding...
a)
Increases
b)
decreases
c)
stays the same
52.
What is EFFECTIVE nuclear charge
a)
The charge that actually matters
b)
The sharge of an element
c)
The charge felt by the valence electrons
d)
The charge felt by the inner orbital electrons
53.
Which of the following elements has the most "shielding" electrons?
a)
Neon
b)
flourine
c)
oxygen
d)
They have the same
54.
Which of the following elements has the lowest amount of shielding electrons?
a)
Argon
b)
Neon
c)
Helium
d)
Radon
55.
Which of the following elements has the largest shielding effect?/
a)
Li
b)
Na
c)
K
d)
Rb
56.
Put the following elements in order of increased shielding effect.
a)
Sodium (Na), Silicon (Si), Chlorine (Cl)
b)
Silicon (Si), Chlorine (Cl), Sodium (Na), 
c)
Chlorine (Cl), Sodium (Na), Silicon (Si)
d)
Each of these has the same amount of shielding.
57.
When shielding increases, it causes 
a)
the atomic radius to increase
b)
the ionization energy to increase
c)
the metallic properties to decrease
d)
the ionic radius to decrease
58.
As you move down a group, shielding 
a)
increases because there are more  orbitals
b)
increases because there are more protons
c)
decreases because the atomic radius increases
d)
stays constant because the number of valence electrons stays the same
59.

Which of the following is the electronic configuration for Mg2+ ion?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p2

d)

1s2 2s2 2p6 3s2

60.

What is the electronic configuration for Phosphorus atom ?

a)

1s22s22p63s23p3

b)

1s22s22p63s23p5

c)

1s22s22p3

d)

1s22s22p63s2

61.

Which one of the following contains no unpaired electrons in the ground state?

a)

Be

b)

F

c)

Si

d)

N

62.

The number of electrons in the 3d orbital of the atom of atomic number 27 is

a)

5

b)

6

c)

7

d)

10

63.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
64.
True or False - Protons and Neutrons have about the same mass.
a)
True - They have about the same mass
b)
False - They do not have about the same mass
65.

Which of the following statements regarding electronic orbitals is/are correct?

a)

Each p-orbital can hold a maximum of six electrons.

b)

The 3p-orbitals have a higher energy level than the 3s-orbital.

c)

The three 3p-orbitals have slightly different energy levels.

d)

The 1s-orbital has the same size and shape as the 2s-orbital.

66.

What is the Aufbau principle?

a)

Within an energy level, s orbitals are the lowest energy, followed by p, d and then f. F orbitals are the highest energy for that level.

b)

The lower the principal quantum number (n) the lower the energy.

c)

All three.

d)

The Aufbau Principle states that electrons enter the lowest energy orbitals first.

67.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
68.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
69.

State the valence electronic configuration for Mg (Z=12)

a)

3s2

b)

3s2 3p1

c)

3s2 3p3

d)

3s2 3p4

70.

Determine the element that has valence electron 3s23p1

(Z of Na = 11, Al = 13, Cl = 17, Mg = 12)

a)

Na

b)

Al

c)

Cl

d)

Mg

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